Consider the following balanced chemical equation. 5 F2 (g)  +  Br2 (l)    →   2 BrF5 (l) 0.789 atm of F2 in a 0.1250 L container at 26.5 °C reacted. How many mol of BrF5 were formed?

Consider the following balanced chemical equation.

5 F_{2 (g)}  +  Br_2 (l)    →   2 BrF_5 (l)

0.789 atm of F₂ in a 0.1250 L container at 26.5 °C reacted. How many mol of BrF₅ were formed?

SHOW WORK. Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Be sure to use our periodic table to calculate any molar masses needed (rounded to proper number of decimal places), otherwise your values might be slightly off and answers may be marked as incorrect. Abbreviate units as follows: grams = g, moles = mol, liters = L, atmospheres = atm

What temperature (with proper s.f.) is entered into the equation? Enter the value in the first blank and the units in the second blank.

Calculate the mol of F₂ reacted (enter value only, with proper s.f.).

 mol

Use the three blanks to enter the number, unit, and substance (in this order) that appears in the denominator of the stoichiometry conversion factor.

Enter the value for the amount of BrF₅ formed (in mol).

 mol